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### Midterm Question

Posted: Wed Feb 20, 2019 6:02 pm
One of the questions asks you to comment on the relative stability of reactants and products. How were you suppose to go about solving this problem?

### Re: Midterm Question

Posted: Wed Feb 20, 2019 6:10 pm
The question basically asks you what the value of the equilibrium constant (K) means. If it is significantly large (>10^3), then that means the reaction favors the right side of the equation, meaning that products are more stable than reactants.

If it's significantly small, then the reactants are more stable than the products.

If the equilibrium constant is around 1, then neither products or reactants are more stable than the other.

### Re: Midterm Question

Posted: Wed Feb 20, 2019 8:05 pm
if K>>>10^3, then products are favored over reactants, and therefore products are more stable.

if K<<<10^-3, then reactants are favored over products, and therefore reactants are more stable.

if K=1, then products and reactants are exactly equally favored, and therefore are equally stable.

for values between 10^-3<<<K<<<10^3, neither products nor reactants are strongly favored.

### Re: Midterm Question

Posted: Wed Feb 20, 2019 9:12 pm
so is the answer that products are more stable

### Re: Midterm Question

Posted: Wed Feb 20, 2019 9:20 pm
yes, because the K value was large so product formation was favored so products are clearly more stable.

### Re: Midterm Question

Posted: Wed Feb 20, 2019 10:06 pm
K is the [P]/[R] so if K is very large, the [P]>[R]. Because the concentration of products is greater at equilibrium, the products must be more stable, because the reaction favors them.